Calculate the volume of oxygen required for complete combustion of 680 g of hydrogen sulfide to oxide.

The oxidation reaction of hydrogen sulfide is described by the following chemical reaction equation.

2H2S + 3O2 = 2H2O + 2SO2;

2 moles of hydrogen sulfide reacts with 3 moles of oxygen. In this case, 2 mol of water and 2 mol of sulfur dioxide are synthesized.

Let’s calculate the chemical amount of hydrogen sulfide.

To do this, we divide its weight by the weight of 1 mole of hydrogen sulfide.

M H2S = 2 +32 = 34 grams / mol; N H2S = 680/34 = 20 mol;

To oxidize such an amount of hydrogen sulphide, 20 x 1.5 = 30 mol of oxygen is required.

Let’s calculate its volume.

To do this, multiply the amount of substance by the volume of 1 mole of gas (22.4 liters).

V O2 = 30 x 22.4 = 672 liters;

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